The equilibrium N2O4(g) 2 NO2(g) is maintained in a closed vessel at 60 deg C and a total pressure of 5 atm, where the observed (average) molar mass of the mixture is 69 g/mol. At the same temperature, at what total pressure would the observed molar mass become 230/3 g/mol?

Question

The equilibrium N2O4(g) <-> 2 NO2(g) is maintained in a closed vessel at 60 deg C and a total pressure of 5 atm, where the observed (average) molar mass of the mixture is 69 g/mol. At the same temperature, at what total pressure would the observed molar mass become 230/3 g/mol?

Accepted Answer

15 atm. From the observed molar masses, alpha = 1/3 at 5 atm and alpha = 0.2 at the unknown pressure; since Kp (= 2.5) is constant at 60 deg C, solving for P gives 15 atm.

The equilibrium N2O4(g) <-> 2 NO2(g) is maintained in a closed vessel at 60 deg C and a total pressure of 5 atm, where the observed (average) molar mass of the mixture is 69 g/mol. At the same temperature, at what total pressure would the observed molar mass become 230/3 g/mol?

Solution

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